Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 23: Problem 17

Write the formulas for each of the following ions and compounds: (a) tetrahydroxozincate(II), (b) pentaaquachlorochromium(III) chloride, (c) tetrabromocuprate(II), (d) ethylenediaminetetraacet atoferrate(II).

Short Answer

Expert verified
The respective formulas; (a) \( \text{Zn(OH)}_4^{2-} \), (b) \( \text{[Cr(H}_2\text{O)}_5\text{Cl]Cl}_2 \), (c) \( \text{CuBr}_4^{2-} \), (d) \( \text{[Fe(edta)]Na}_4 \)

Step by step solution

01

Tetrahydroxozincate(II)

Tetrahydroxozincate(II) indicates that zinc forms a complex ion with 4 hydroxide ions and its charge is 2-. Thus, the ion formula is \( \text{Zn(OH)}_4^{2-} \)
02

Pentaaquachlorochromium(III) chloride

Pentaaquachlorochromium(III) chloride indicates that a chromium ion with a charge of +3 is surrounded by 5 water molecules in complex, also there is one chloride. The complex ion is \( \text{[Cr(H}_2\text{O)}_5\text{Cl]}^{2+} \) and the compound formula is \( \text{[Cr(H}_2\text{O)}_5\text{Cl]Cl}_2 \)
03

Tetrabromocuprate(II)

Tetrabromocuprate(II) indicates that copper forms a complex ion with 4 bromide ions and its charge is 2-. Thus, the ion formula is \( \text{CuBr}_4^{2-} \)
04

Ethylenediaminetetraacetatoferrate(II)

Ethylenediaminetetraacetatoferrate(II) indicates that a ferrous ion is in a complex with an ethylenediaminetetraacetate ion. The EDTA ion usually has 4- charge. So, in order to balance the charge, four sodium ions will be present. So the formula is \( \text{[Fe(edta)]Na}_4 \)

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Chemical analysis shows that hemoglobin contains 0.34 percent of Fe by mass. What is the minimum possible molar mass of hemoglobin? The actual molar mass of hemoglobin is about 65,000 g. How do you account for the discrepancy between your minimum value and the actual value?

The \(\mathrm{Co}^{2+}\) -porphyrin complex is more stable than the \(\mathrm{Fe}^{2+}\) -porphyrin complex. Why, then, is iron the metal ion in hemoglobin (and other heme-containing proteins)?

Predict the number of unpaired electrons in the following complex ions: (a) \(\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{4-},(\mathrm{b})\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\)

Why do transition metals have more oxidation states than other elements?

Explain why a thermodynamically stable species may be chemically reactive and a thermodynamically unstable species may be unreactive.
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free